To gain a better understanding of the typical reaction of the addition of two binary compounds, and how the reaction of those two compounds can be predicted. III. Variables: ==>Dependent Variable: Reagents given, hence the solutions we make from these reagents, and the standard solubility rules. ==>Controlled Variables: The two reagents which we will react together at each trial. ==>Independent Variable: Whether the reagents will create a precipitate or not, which depends on the reagents combined. IV. Hypothesis: If the compound is containing mettle and is added to a compound that is also containing mettle.
The two mettles will change places and then something in the equation will precipitate out of the solution. The majority of the elements will not precipitate and none will have a whole solution of precipitant. All will have some form of ion solution that we are left over from the chemical reaction. V. Materials: o Compounds.
Stirring rod VI. Procedure: 1. Prepare 1 molar solutions of given reagents: i.
Calculate amounts to combine of given reagents. Complete the following for all 16 reagents: 1. As you need 5 ml of solution, begin with this amount 2. Multiply by the molar amount which you wish to use for the reactions. 3. Multiply by the molecular mass of the given compound.
4. This will give you the amount, in grams, of the molecule for which you are calculating. ii. Create 1 molar reagents. Complete the following for each reagent: 1. Mark 16 – 10 ml flasks with masking tape showing the content, showing each of the 16 reagents – one for each flask.
2. Measure out the amount, which you calculated in the Part a, of the reagent. 3. Place this mass of the reagent into the flask which is marked with the reagent. 4. Measure out 5 ml of distilled water in the 10 ml graduated cylinder, and place this water in the flask with the reagent. 5. Stir the reagent so as to combine it completely. 2. Combine given reagents. i. Grid a transparency so that each reagent has a chance to react with every other reagent. Also make a data chart to write in the data which you will collect. ii. Complete the following for each solution: iii.
Take one to two drops of the solution and place it in all the boxes which are marked on your grid transparency. iv. After all solutions have been combined, write in your data chart whether a precipitant has formed, and if so, describe the precipitant; describe the composition of the solution. 3. Evaluate results: i. Write the balanced equations for each of the reactions which occurred in this experiment. ii. Use solubility rules to determine if a precipitant has formed in each reaction. Conclusion and Evaluation: My hypothesis, “If the compound is containing mettle and is added to a compound that is also containing mettle.
The two mettles will change places and then something in the equation will precipitate out of the solution. The majority of the elements will not precipitate and none will have a whole solution of precipitant. All will have some form of ion solution that we are left over from the chemical reaction. ” Was correct. The statement that I made was correct but at the time of the hypothesis I could not comprehend the complexity and the knowledge that would come out of a few simple and harmless experiments, such as this. Thus looking back I feel that I could have written a more complex and informative hypothesis.
When asked to classify the outcomes and pieces of the experiment as qualitative or quantitative I came up with this. The qualitative aspects of this lab have a wide range. The first would be the colors themselves. With each different in its own way it is possible to distinguish certain chemical reaction from other chemical reactions. The qualitative data for this lab would include the chemical formulas. It would also include the mathematical calculations of precipitants. There was also the mathematical calculation that was required to determine the correct ratio that needed to be combined to create the solutions.
This math needed to be conducted with great precision and accuracy. One way in which this experiment could be improved would be to limit the sources of error that were present throughout the experiment. The first would be to use greater quantities of the solutions so the reaction could be better observed. Threw the use of a larger quantity of solution I could have mixed the elements in a flask thus producing a more observable and a more accurate observation. This type of experiment continuity is vital in order to derive any factual conclusions about the chemical bonding of different elements.
Next time around some interesting paths to take from this experiment would be to expand the chemical testing to more elements such as some more exotic compounds. It would also be interesting to observe the nature of some things like pesticides such as acephate (C4H10NO3PS) and also the nature of the very versatile and commonly used element Hg. The experiment was quite informative of the chemical nature of simple elements and how it works. It also brought about a realization of how much work and chemistry really goes into the everyday chemical reactions.